# Question d4d89

$\text{Hydrogen chloride}$ would BEHAVE MUCH LESS ideally than $\text{helium......}$
Ideality assumes minimal interaction between the gaseous particles. For $\text{hydrogen chloride}$, a potent intermolecular force can operates: $\text{hydrogen bonding}$, in that the hydrogen is bound to a strongly electronegative chlorine to give the ""^(-delta)Cl-H^(delta+)# dipole, which can act intermolecularly.
Possibly the best metric with which to compare this is the boiling point of the gases: helium has a normal boiling point of $4 \cdot K$; hydrogen chloride boils at $188 \cdot K$ $-$ how is this consistent with the hydrogen bonding argument? Compare also normal the boiling point of $H F$, where hydrogen bonding should be stronger or weaker than in $H C l$?
AS hydrogen chloride also possesses many more electrons than does helium, dispersion forces will also be stronger for $H C l$.